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Chemistry Exam III

Total questions: 60

Worksheet time: 15hrs 0mins

Name
Class
Date
1.

If you need 10.0 moles of sucrose, how many liters of a 4.0 molar solution would you need?

a)

2.5L

b)

0.25L

c)

10.0L

d)

25L

e)

None of the above

2.

Why might a solvent like turpentine be better for removing grease and grime than water?

a)

Water is too polar and doesn’t interact with the nonpolar oils

b)

Oil and grease have similar interatomic forces as the turpentine and so are more soluble

c)

Oil and grease have very similar solubility in the water

d)

like dissolves like

e)

All of the above

3.

Which of the following solutions is most dilute?

a)

One liter of water with 5 grams of sugar

b)

One liter of water with 1 gram of sugar

c)

One liter of water with 10 grams of sugar

d)

One liter of water with 2 grams of sugar

e)

They all have the same volume

4.

Which of the following would have the most induced dipole attractions between itself in the pure sample?

a)

C6H14

b)

C12H26

c)

C8H18

d)

C10H22

e)

Not enough information given

5.

Chlorine , Cl2, is a gas at room temperature, but bromine Br2, is a liquid. Explain.

a)

Bromine atoms are larger and this makes the formation of induced dipole—induced dipole attractions more favorable

b)

Chlorine atoms are larger and this makes the formation of induced dipole—induced dipole attractions more favorable

c)

The smaller chlorine molecules are able to pack together in tighter physical orientation

d)

The bromine ions are held together by ionic bonds

6.

Which of the following bonds will be the most polar?

a)

C-Br

b)

C-F

c)

C-Cl

d)

C-I

e)

All are equally polar

7.

How many molecules of sucrose are in 0.500L of a 1.00 molar solution of sucrose?

a)

1 gram

b)

0.5

c)

3.01 x 1023 molecules of sucrose

d)

6.02 x 1023 molecules of sucrose

e)

12.04 x 1023 molecules of sucrose

8.

For the following reaction, identify whether the compound underlined is behaving as an acid or a base.

H3PO4 + H2O = H2PO4 + H3O+

a)

Acid

b)

Base

c)

Neither

d)

Both

9.

  What is a base?

a)

Anything that can be used to clean drains

b)

Anything that donates a proton

c)

Anything that accepts a proton

d)

Anything that can be used to make soap

e)

Anything that has a bitter taste

10.

How do you take a proton out of a hydrogen atom?

a)

Let the hydrogen atoms undergo fusion

b)

Remove a proton from a helium nucleus

c)

Remove an electron from a hydrogen atom

d)

Let the hydrogen atoms combine to form a hydrogen molecule and eject an electron

e)

Let the hydrogen atoms combine to form a hydrogen molecule and eject a proton

11.

According to the following reaction, which molecule is acting as an acid?

H2O + NH3 --> OH- +NH4+

a)

NH4+

b)

H2O

c)

OH-

d)

NH3

e)

None of the above

12.

For the following acid-base reaction, identify what compound is formed in the space marked.

HCl + KOH= ???? +H2O

a)

K3OCl

b)

KOH2

c)

KOH2Cl

d)

KCl

e)

none of the above

13.

Qualitatively, what happens to the hydroxide ion concentration if you decrease the hydronium ion concentration?

a)

The concentration of hydroxide decreases to neutralize the excess hydronium

b)

The concentration of OH—increases

c)

The concentration of OH- stays the same but the ratio OH‑/H3­O+ changes

d)

The concentration of OH- increase but the ratio stays the same

e)

None of the above

14.

Which of the following is the most acidic?

a)

A solution with pH=7

b)

A solution with pH=10

c)

A solution with pH=4

d)

A solution with pH=14

e)

All of the solutions are basic

15.

Which is higher in endothermic reaction: the potential energy of the reactants or the potential energy of the products?

a)

The potential energy of the reactants is the same as the potential energy of the products

b)

The potential energy of the products is higher than the potential energy of the reactants

c)

The potential energy of the reactants is higher than the potential energy of the products

d)

In the early stages of the reaction the potential energy of the reactants is higher, In the late stages, the potential energy of the products is higher

16.

Under which of the following conditions would you expect the highest solubility of oxygen gas in water?

a)

High temperature and high O­2 pressure above the solution

b)

Low temperature and low O2­ pressure above the solution

c)

High temperature and low O2 pressure above the solution

d)

Low temperature and high O2­ pressure above the solution

e)

The O2  solubility is independent of temperature and pressure

17.

What is (are) the main characteristic(s) of a strong acid?

a)

It will damage your skin

b)

It readily gives up its proton to a base

c)

It is corrosive

d)

It is completely disassociated in water

e)

All of the above

18.

Given the above energy profiles have the same scale, which of the reactions is the most exothermic?

a)

A

b)

B

c)

C

d)

D

e)

None of the above

19.

Which of the following has the greatest mass?

a)

1 mole Na

b)

1 mole of Be

c)

1 mole of H2

d)

1 mole of Pb

e)

All have the same mass

20.

How does a catalyst increase the rate of reaction?

a)

It lowers the activation energy

b)

It raises the activation energy of the reactants, which makes the reaction proceed faster

c)

It has nothing to do with the rate of reaction

d)

  It increases the energy difference between the reactants and products

e)

  It is neither created nor consumed in a reaction

21.

Which has more atoms: 64.508g of sulfur dioxide, SO2 (64.058 amu), or 72.922 g of hydrogen chloride, HCl (36.461 amu)?

a)

72.922 g HCl and 64.058g of SO2 have above the same number of atoms

b)

72.922g of HCl has more atoms than 64.058g of SO2

c)

64.058g of SO2 has more atoms than 72.922g of HCl

d)

Not enough information is given

 

22.

According to the following balanced chemical equation, if you want to generate 2 moles of H2O how many grams of O2 do you need?

2H2 + O2 --> 2H2O

a)

16

b)

8

c)

4

d)

6.022 x 1023

e)

32

23.

What coefficient is needed in front of the O2 molecule to balance the following equation?

P4+ ___ O2----> P4O10

a)

5

b)

10

c)

8

d)

1

24.

Small samples of oxygen gas needed in the laboratory can be generated by any number of simple chemical reactions, such as:

2KClO3 (s) ----> 2KCl (s) + 3O2 (g)

What masses of oxygen (in grams) is produced when 122.6g of KClO3 (formula mass=122.6amu) takes part in this reaction?

a)

48.00 grams

b)

96.00 grams

c)

32.00 grams

d)

More information is needed

25.

What is the number of moles of H2O produced if you combust 0.5 mole of CH4 according to the following balanced equation?

CH4 + 2O2--->CO2 +2H2O

a)

2 moles

b)

4 moles

c)

1 mole

d)

6 moles

e)

8 moles

26.

  Given that the above energy profiles have the same scale, which of the reactions would require the most energy?

a)

A

b)

B

c)

C

d)

D

e)

None of the above

27.

How many oxygen molecules are needed to make 10 carbon dioxide molecules according to the following balanced chemical equation:

2CO +O­2 ---> 2CO2

a)

1

b)

5

c)

10

d)

2

e)

4

28.

What is a reaction rate?

a)

It is the speed at which reactants are consumed or product is formed

b)

It is the ratio of the molecular masses pf the elements in a given compound

c)

It is the ratio of the masses of products and reactants

d)

It is the balance chemical formula that relates the number of product molecules to reactant molecules

e)

None of the above

29.

What is the formula mass of sulfur dioxide, SO2 ?

a)

About 16 amu

b)

About 60 amu

c)

About 32 amu

d)

About 64 amu

30.

What is a chemical reaction?

a)

When a liquid undergoes a phase change and produces a solid

b)

When two liquids mix to form a homogeneous mixture

c)

When a new element is formed by rearranging nucleons

d)

When one or more new compounds are formed by rearranging atoms

e)

When two solids mix together to form an heterogeneous mixture

31.

Which of the following has the greatest number of particles?

a)

One mole of Na

b)

9.12 g of Be

c)

1 mole of Be

d)

22.990g of Na

e)

All are the same

32.

True or False: H2O is nonpolar?

a)

T

b)

F

33.

True of false: Methane is polar

a)

F

b)

T

34.

Is HNO polar, nonpolar, ionic, or metallic

a)

polar

b)

nonpolar

c)

ionic

d)

metallic

35.

Determine the following Molecular Attraction between: H2O and CCl4

a)

Ion-Dipole

b)

Dipole-Dipole

c)

Dipole-Induced Dipole

d)

Induced Dipole-Induced Dipole

36.

Determine the following Molecular Attraction between: NF3 and BF3

a)

Ion-Dipole

b)

Dipole-Dipole

c)

Dipole-Induced Dipole

d)

Induced Dipole-Induced Dipole

37.

Determine the following Molecular Attraction between: Methane and HC

a)

Ion-Dipole

b)

Dipole-Dipole

c)

Dipole-Induced Dipole

d)

Induced Dipole-Induced Dipole

38.

Determine the following Molecular Attraction between: Potassium and H2S

a)

Ion-Dipole

b)

Dipole-Dipole

c)

Dipole-Induced Dipole

d)

Induced Dipole-Induced Dipole

39.

Determine the following Molecular Attraction between: NH3 and H2O

a)

Ion-Dipole

b)

Dipole-Dipole

c)

Dipole-Induced Dipole

d)

Induced Dipole-Induced Dipole

40.

Determine the following Molecular Attraction(s) between: HF and H2O

a)

Ion-Dipole

b)

Dipole-Dipole

c)

Dipole-Induced Dipole

d)

Induced Dipole-Induced Dipole

e)

Hydrogen Bonding

41.

In a 5g of salt and 75g of water are mixed which is the solvent

a)

Salt

b)

Water

42.

1 oz. of chocolate syrup and 8 oz. of milk are mixed which is the solute

a)

chocolate syrup

b)

milk

43.

8 cups of tea and ¼ cups of sugar are mixed which is the solute

a)

Tea

b)

Sugar

44.

Which is more concentrated: 15g of sugar in 300g of tea OR 15g of sugar 150g of tea

a)

15g of sugar in 300g of tea

b)

15g of sugar 150g of tea

45.

identify which is more concentrated: 10g of salt in 100mL of water OR 10g of salt in 150mL of water

a)

10g of salt in 150mL of water

b)

10g of salt in 100mL of water

46.

12 moles of salt dissolved into 6 liters of water. What is the molarity?

a)

0.5

b)

2

c)

72

d)

none of the above

47.

A solution consists of 7 moles of sugar and has a molarity of 21. How many liters are in the solution?

a)

1/3

b)

3

c)

147

d)

none of the above

48.

A solution has a molarity of 3 and consists of 2 liters of water. How many molecules are in the solution?

a)

6

b)

0.66666

c)

1.5

d)

36.12x1023

49.

Balance the following equation:

__ Li2SO4 + __ K3PO4 = __ Li3PO4 + __ K2SO4

a)

3,2,2,3

b)

2,1,1,2

c)

1, 2, 1, 4

d)

1,3,3,1

50.

Balance the following equation:

__ Al +__ O2 = __ Al2O3

a)

1,2,3

b)

8,16,1

c)

2,1,1

d)

4,3,2

51.

1.     Balance this equation:

            __ CH4 + __ O2 = __ CO2 + __ H2O

If you have 8g of methane, how many grams of oxygen do you need to fully react the methane?

a)

32

b)

4

c)

1

d)

0.5

52.

Balance the following equation:

__ N2 + __ H2 = __ NH3

 If you have 8 moles of ammonia, how many moles of hydrogen did you start out with?

a)

24

b)

26

c)

12

d)

18

53.

Balance the following equation:

__ H2O + __ CO = __ CO2 + __ H2

How many grams of water do you need to get 0.5 moles of carbon dioxide?

 

a)

0.5

b)

9

c)

0.02778

d)

36

54.

identify the acid in the following equation:

H2SO4 + OH = HSO4 + H2O

a)

H2SO4

b)

OH

c)

HSO4

d)

H2O

55.

identify the base in the following equation:

C2H3O2 + H2O = OH + HC2H3O2

a)

H2O

b)

C2H3O2

c)

OH

d)

HC2H3O2

56.

If a solution has a hydronium concentration of [H3O+] > 1x10-7M does that make the solution acidic, basic, or neutral?

a)

Basic

b)

Acidic

c)

Neutral

57.

if a solution has a hydroxide concentration of [OH-] > 1x10-7M is the solution acid, basic, or neutral?

a)

Acidic

b)

Basic

c)

Neutral

58.

if a solution has the following hydroxide and hydronium concertation [H3O+]=[OH-]= 1.0 x 10-7 M is the solution acidic, basic, or neutral?

a)

Basic

b)

Acidic

c)

Neutral

59.

if a solution where to have a pH of 9 would it be acidic, basic, or neutral?

a)

Basic

b)

Acidic

c)

Neutral

60.

If a solution were to have a pH of 6.9 would the solution be acidic, basic, or neutral?

a)

Acidic

b)

Basic

c)

Neutral

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